E°zn2-/z0) = -0.763 V MMz = 65.38 g/mol Zn2+(aq) +2e--Zn(s) a.) If a current of 35.0 amps flows for 5.00 minutes through this solution, how many moles of electrons have moved through the solution? ( b.) How many grams of zinc can be produced using a current of 0.40 amps for 0.75 hours?

E°zn2-/z0) = -0.763 V MMz = 65.38 g/mol Zn2+(aq) +2e--Zn(s) a.) If a current of 35.0 amps flows for 5.00 minutes through this solution, how many moles of electrons have moved through the solution? ( b.) How many grams of zinc can be produced using a current of 0.40 amps for 0.75 hours?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 128AE: It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

E°zn2-/za) = -0.763 V
MMzn = 65.38 g/mol
Zn2+(aq)
+2e--Zn(s)
a.) If a current of 35.0 amps flows for 5.00 minutes through this solution, how many moles of
electrons have moved through the solution? (
b.) How many grams of zinc can be produced using a current of 0.40 amps for 0.75 hours?

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